Question

In: Chemistry

At a temp below room temp but with all components as gases, the decomposition of iodine...

At a temp below room temp but with all components as gases, the decomposition of iodine monochloride, ICl, to iodine and chlorine, is 1.4*10^-5

2ICl (g)----> I2 (g) + Cl2 (g)

If a sealed vessel has [ICl]=1.87 M, and no iodine or chlorine. What are the equilibrium cocentrations?

Expert Solution

2ICl (g) I₂ (g) + Cl₂ (g)

initial conc.(M) 1.87 0 0

change -2a +a +a

Equb conc(M) 1.87-2a a a

Equilibrium constant , K_c = ([I₂ (g)] [Cl₂ (g)]) / [ICl]²

1.4x10^-5 = (a x a ) / (1.87-2a)²

1.4x10^-5 = a² / (1.87-2a)²

a / (1.87-2a) = 3.74x10^-3

a = 6.997x10^-3 - 7.48x10^-3 a

8.48x10^-3 a = 6.997x10^-3

a = 6.94x10^-3 M

So Equilibrium concentration of I₂ (g) = Cl₂ (g) = a = 6.94x10^-3 M

Equilibrium concentration of ICl (g) = 1.87-2a

= 1.87 -(2x6.94x10^-3 )

= 1.86 M

queen_honey_blossom answered 2 years ago

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